Advertisements
Advertisements
प्रश्न
Briefly give the basis for Pauling's scale of electronegativity.
उत्तर
Pauling’s scale:
- Electronegativity is the relative tendency of an element present in a covalently bonded molecule to attract the shared pair of electrons towards itself.
- Pauling assigned arbitrary values of electronegativities for hydrogen and fluorine as 2.2 and 4, respectively.
- Based on this the electronegativity values for other elements can be calculated using the following expression.
(XA − XB) = `0.182 sqrt("E"_"AB" - ("E"_"AA" xx "E"_"BB")^(1/2))`
Where EAB, EAA, and EBB are the bond dissociation energies of AB, A2, and B2 molecules respectively.
XA and XB are electronegativity values of A and B.
APPEARS IN
संबंधित प्रश्न
Which of the following elements will have the highest electronegativity?
The element with positive electron gain enthalpy is
The electronic configuration of the atom having maximum difference in first and second ionisation energies is
What is the effective nuclear charge?
Magnesium loses electrons successively to form Mg+, Mg2+ and Mg3+ ions. Which step will have the highest ionisation energy and why?
In what period and group will an element with Z = 118 will be present?
Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium?
By using Pauling's method calculate the ionic radii of K+ and Cl− ions in the potassium chloride crystal. Given that `"d"_("K"^+) - "Cl"^-` = 3.14 Å
Explain the following, give an appropriate reason.
The formation of \[\ce{F^-_{(g)}}\] from \[\ce{F_{(g)}}\] is exothermic while that of \[\ce{O^2-_{(g)}}\] from \[\ce{O_{(g)}}\] is endothermic.
State the trends in the variation of electronegativity in groups and periods.
